The equation for the reaction is 2 Na S2 O3 (aq) + 2HCl(aq) o 2NaCl(aq) + H2 O(l) + S(s) + SO2 (g) Before starting her experiments, the student considers the risk to her of sulfur dioxide escaping from the flask. She uses this information. concentration of sodium thiosulfate solution = 0.300 mol/dm3 volume of sodium thiosulfate solution = 20 cm3 volume of water = 20 cm3 volume of hydrochloric acid = 10 cm3 The solubility of sulfur dioxide at room temperature is 100 g/dm3. Use this additional information to explain whether any sulfur dioxide gas escapes from the flask.
Question
The equation for the reaction is 2 Na S2 O3 (aq) + 2HCl(aq) o 2NaCl(aq) + H2 O(l) + S(s) + SO2 (g) Before starting her experiments, the student considers the risk to her of sulfur dioxide escaping from the flask. She uses this information. concentration of sodium thiosulfate solution = 0.300 mol/dm3 volume of sodium thiosulfate solution = 20 cm3 volume of water = 20 cm3 volume of hydrochloric acid = 10 cm3 The solubility of sulfur dioxide at room temperature is 100 g/dm3. Use this additional information to explain whether any sulfur dioxide gas escapes from the flask.
Solution
To determine whether any sulfur dioxide gas escapes from the flask, we first need to calculate the amount of sulfur dioxide produced in the reaction.
From the balanced chemical equation, we can see that 2 moles of sodium thiosulfate react with 2 moles of hydrochloric acid to produce 1 mole of sulfur dioxide.
Given that the concentration of sodium thiosulfate solution is 0.300 mol/dm3 and the volume of the solution is 20 cm3, we can calculate the number of moles of sodium thiosulfate in the solution as follows:
Number of moles = concentration x volume = 0.300 mol/dm3 x 20 cm3 = 0.006 mol
Since the ratio of sodium thiosulfate to sulfur dioxide in the reaction is 2:1, the number of moles of sulfur dioxide produced is half the number of moles of sodium thiosulfate, which is 0.003 mol.
The molar mass of sulfur dioxide is approximately 64 g/mol, so the mass of sulfur dioxide produced in the reaction is:
Mass = number of moles x molar mass = 0.003 mol x 64 g/mol = 0.192 g
Given that the solubility of sulfur dioxide at room temperature is 100 g/dm3, this means that up to 100 g of sulfur dioxide can be dissolved in 1 dm3 (or 1000 cm3) of water at room temperature.
Since the volume of water in the flask is 20 cm3, the maximum amount of sulfur dioxide that can be dissolved in the water is:
Maximum mass = solubility x volume = 100 g/dm3 x 20 cm3 = 2 g
Since the mass of sulfur dioxide produced in the reaction (0.192 g) is less than the maximum amount that can be dissolved in the water (2 g), it is unlikely that any sulfur dioxide gas will escape from the flask.
Similar Questions
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